The straight lines in the figure depict the variations in temperature `DeltaT` as a function of the amount of heat supplied `Q` is different process involving the change of state of a monoatomic and a diatomic ideal gas . The initial states, (`P,V,T`) of the two gases are the same . Match the processes as described, with the straight lines in the graph as numbered.

`{:(,"Column-I",,"Column-II"),((A),"Isobaric process of monoatomic gas." ,(p),"1" ),((B),"Isobaric process of diatomic gas" ,(q),"2" ),((C),"Isochoric process of monoatomic gas" ,(r),"Minimum at section B"), ((D),"Isochoric process of diatomic gas" ,(s),"x-axis (i.e.'Q' axis)"):}`

Explanation

As `Q = mCdt` and `dT = (Q)/(nC)`
Therefore molar heat constant `C` is the determining factor for rate of change of temperature of a gas as heat is supplied to it. It is minimum for isochoric process of a monoatomic gas `(C_(V) = (3)/(2)R)`, resulting in greatest slope `((dT)/(Q))` i.e.curve `1`.
For isobaric process of monoatomic gas and isochoric process of diatomic gas, their heat capacities are same `((5)/(2)R)` ,therefore both are represented by curve `2` .
For isobaric process of diatomic gas `C_(p) = (7)/(2)R` that is represented by curve `3. Q` axis represent by curve isothermal process and `DeltaT` axis represent adiabatic process.